Question

In reality, N2O is used to supplement O2 during combustion. However, for this problem, assume that all of the O2 required for combustion is supplied by decomposition of N2O. In this scenario, what volume of octane (density = 0.700 g/mL) can be burned using a NOS canister containing 10.0 lb (1.00 lb = 0.454 kg) of N2O? Hint: Start by writing a balanced equation for the decomposition of N2O to N2 and O2 and for the combustion of octane.

A.

1350 mL

B.

673 mL

C.

16.8 L

D.

330 mL

Answer 1

Solution:-

Solution Desomposthon weigh mole 540 lo 3.15 moli lequvelin 02 u 103.15 moles moles 51.58 mole uanon bun 2 moles oles

Now density = mass/ volume so volume = mass / density [ densit given = 0.700 g /mL ]

volume = 471.23/ 0.700 = 673 mL

volume of octane = 673 mL